Unit 11 Practice Test

Name: ________________________ Class: ___________________ Date: __________
ID: A
Unit 11 Practice
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
1) Crystalline solids ____.
A) have their particles arranged randomly
B) have highly ordered structures
C) are usually very soft
D) exist only at high temperatures
E) exist only at very low temperatures
____
2) Together, liquids and solids constitute ____ phases of matter.
A) the compressible
B) the fluid
C) the condensed
D) all of the
E) the disordered
____
3) When NaCl dissolves in water, aqueous Na+ and Cl– ions result. The force of attraction that exists between Na +
and H2O is called a(n) ____ interaction.
A) dipole-dipole
B) ion-ion
C) hydrogen bonding
D) ion-dipole
E) London dispersion force
____
4) Elemental iodine (I2) is a solid at room temperature. What is the major attractive force that exists among
different I2 molecules in the solid?
A) London dispersion forces
B) dipole-dipole rejections
C) ionic-dipole interactions
D) covalent-ionic interactions
E) dipole-dipole attractions
____
5) C12H26 molecules are held together by ____.
A) ion-ion interactions
B) hydrogen bonding
C) ion-dipole interactions
D) dipole-dipole interactions
E) dispersion forces
____
6) What type(s) of intermolecular forces exist between Br 2 and CCl4?
A) dispersion forces
B) dispersion forces and ion-dipole
C) dispersion forces and dipole-dipole
D) dispersion forces, ion-dipole, and dipole-dipole
E) None. Since both are gases at room temperature, they do not interact with each other.
1
Name: ________________________
ID: A
____
7) The shape of a liquid's meniscus is determined by ____.
A) the viscosity of the liquid
B) the type of material the container is made of
C) the relative magnitudes of cohesive forces in the liquid and adhesive forces between the
liquid and its container
D) the amount of hydrogen bonding in the liquid
E) the volume of the liquid
____
8)
The phase changes B  C and D  E are not associated with temperature increases because the heat energy
is used up to ____.
A) increase distances between molecules
B) break intramolecular bonds
C) rearrange atoms within molecules
D) increase the velocity of molecules
E) increase the density of the sample
____
9) The substance with the largest heat of vaporization is ____.
A) I2
B) Br2
C) Cl2
D) F2
E) O2
____ 10) Volatility and vapor pressure are ____.
A) inversely proportional to one another
B) directly proportional to one another
C) not related
D) the same thing
E) both independent of temperature
2
Name: ________________________
ID: A
____ 11) On a phase diagram, the melting point is the same as ____.
A) the triple point
B) the critical point
C) the freezing point
D) the boiling point
E) the vapor-pressure curve
____ 12) Which of the following characteristics would prevent liquid crystal behavior?
A) long axial structure
B) ionic configuration
C) carbon-carbon single bonds
D) double bonding
E) polar groups
____ 13) In the ____ liquid crystalline phase, the component molecules exhibit only one dimensional ordering.
A) nematic
B) smectic A
C) smectic B
D) smectic C
E) cholesteric
____ 14) Based on molecular mass and dipole moment of the five compounds in the table below, which should have the
highest boiling point?
A)
B)
C)
D)
E)
CH3CH2CH3
CH3OCH3
CH3Cl
CH3CHO
CH3CN
3
Name: ________________________
ID: A
____ 15) The heating curve shown was generated by measuring the heat flow and temperature for a solid as it was heated.
The slope of the ____ segment corresponds to the heat capacity of the solid.
A) AB
B) BC
C) CD
D) DE
E) EF
____ 16) On the phase diagram shown above, the coordinates of point ____ correspond to the triple point.
A) A
B) B
C) C
D) D
E) E
4
Name: ________________________
ID: A
____ 17) The phase diagram of a substance is shown above. The area labeled ____ indicates the gas phase for the
substance.
A) w
B) x
C) y
D) z
E) y and z
____ 18) According to the phase diagram shown above, the normal melting point of this substance is ____ °C.
A) –13
B) 10
C) 29
D) 38
E) 0
____ 19) Which type of liquid crystal is colored and changes color with temperature?
A) nematic
B) smectic A
C) cholesteric
D) smectic B
E) smectic C
____ 20) With what compound will NH3 experience only ion-dipole intermolecular forces?
A) LiCl
B) SiH4
C) CH3I
D) C3H7OH
E) OCl2
____ 21) Which one of the following exhibits dipole-dipole attraction between molecules?
A) NH3
B) CF4
C) C10H22
D) O2
E) SF6
5
Name: ________________________
ID: A
____ 22) Which one of the following should have the lowest boiling point?
A) CH4
B) PCl3
C) C2H5COOH
D) LiCl
E) Cl2S
____ 23) What is the predominant intermolecular force in H2NNH2?
A) hydrogen bonding
B) ion-dipole attraction
C) ionic bonding
D) dipole-dipole attraction
E) London-dispersion forces
____ 24) The heat of fusion of water is 6.01 kJ/mol. The heat capacity of liquid water is 75.3 J/mol  K. The conversion
of 50.0 g of ice at 0.00 °C to liquid water at 0.00°C requires ____ kJ of heat.
A) 6.01
B) 16.7
C) 75.3
D) 17.2
E) Insufficient data are given.
____ 25) Of the following, ____ is the least volatile.
A) CI4
B) CF4
C) CBr4
D) CCl4
E) CH4
6
Name: ________________________
ID: A
____ 26) Based on the figure above, the boiling point of ethyl alcohol under an external pressure of 0.658 atm is ____
°C.
A) 20
B) 40
C) 60
D) 80
E) 70
Short Answer
1) In general, intramolecular forces determine the ________ properties of a substance and intermolecular forces
determine its ________ properties.
2) London Dispersion Forces tend to ________ in strength with increasing molecular weight.
3) The direct conversion of a solid to a gas is called ________.
4) The initial discovery of a liquid crystal resulted from studies on what compound?
True/False
Indicate whether the statement is true or false.
____
1) The principal source of the difference in the normal boiling points of ICl (97 °C; molecular mass 162 amu) and
Br2 (59 °C; molecular mass 160 amu) is both dipole-dipole interactions and London dispersion forces.
7
Name: ________________________
ID: A
____
2) The boiling points of normal hydrocarbons are higher than those of branched hydrocarbons of similar
molecular weight because the London-dispersion forces between normal hydrocarbons are greater than those
between branched hydrocarbons.
____
3) Heats of vaporization are greater than heats of fusion.
____
4) Under ordinary conditions, a substance will sublime rather than melt if its triple point occurs at a pressure above
atmospheric pressure.
____
5) Molecules containing only single bonds do not exhibit liquid-crystal behavior because free rotation can occur
around single bonds making these molecules flexible.
8
ID: A
Unit 11 Practice
Answer Section
MULTIPLE CHOICE
1) ANS:
OBJ:
2) ANS:
OBJ:
3) ANS:
OBJ:
4) ANS:
OBJ:
5) ANS:
OBJ:
6) ANS:
OBJ:
7) ANS:
OBJ:
8) ANS:
OBJ:
9) ANS:
OBJ:
10) ANS:
OBJ:
11) ANS:
OBJ:
12) ANS:
OBJ:
13) ANS:
OBJ:
14) ANS:
OBJ:
15) ANS:
OBJ:
16) ANS:
OBJ:
17) ANS:
OBJ:
18) ANS:
OBJ:
19) ANS:
OBJ:
20) ANS:
OBJ:
21) ANS:
OBJ:
B
PTS:
G2
C
PTS:
G2
D
PTS:
11.2; G2
A
PTS:
11.2; G2
E
PTS:
11.2; G2
A
PTS:
11.2; G2
C
PTS:
11.3; G2
A
PTS:
11.4; G3
A
PTS:
11.4; G2
B
PTS:
11.5, 11.6; G2
C
PTS:
11.6; G2
B
PTS:
11.7; G2
A
PTS:
11.7; G2
E
PTS:
11.2; G3
A
PTS:
11.4; G3
A
PTS:
11.5, 11.6; G3
C
PTS:
11.5, 11.6; G3
E
PTS:
11.5, 11.6; G3
C
PTS:
11.7; G2
A
PTS:
11.2; G2
A
PTS:
11.2; G2
1
DIF: 1
REF: Page Ref: 11.1
1
DIF: 1
REF: Page Ref: 11.1
1
DIF: 2
REF: Page Ref: 11.2
1
DIF: 2
REF: Page Ref: 11.2
1
DIF: 2
REF: Page Ref: 11.2
1
DIF: 3
REF: Page Ref: 11.2
1
DIF: 2
REF: Page Ref: 11.3
1
DIF: 3
REF: Page Ref: 11.4
1
DIF: 2
REF: Page Ref: 11.4
1
DIF: 2
REF: Page Ref: 11.5
1
DIF: 1
REF: Page Ref: 11.6
1
DIF: 1
REF: Page Ref: 11.7
1
DIF: 5
REF: Page Ref: 11.7
1
DIF: 3
REF: Page Ref: 11.2
1
DIF: 1
REF: Page Ref: 11.4
1
DIF: 2
REF: Page Ref: 11.6
1
DIF: 2
REF: Page Ref: 11.6
1
DIF: 2
REF: Page Ref: 11.6
1
DIF: 1
REF: Page Ref: 11.7
1
DIF: 2
REF: Page Ref: 11.2
1
DIF: 3
REF: Page Ref: 11.2
1
ID: A
22) ANS:
OBJ:
23) ANS:
OBJ:
24) ANS:
OBJ:
25) ANS:
OBJ:
26) ANS:
OBJ:
A
PTS:
11.2; G2
A
PTS:
11.2; G2
B
PTS:
11.4; G4
D
PTS:
11.5, 11.6; G2
E
PTS:
11.5, 11.6; G3
1
DIF: 3
REF: Page Ref: 11.2
1
DIF: 2
REF: Page Ref: 11.2
1
DIF: 4
REF: Page Ref: 11.4
1
DIF: 2
REF: Page Ref: 11.5
1
DIF: 3
REF: Page Ref: 11.5
SHORT ANSWER
1) ANS:
chemical, physical
PTS: 1
OBJ: G2
2) ANS:
increase
DIF: 2
REF: Page Ref: 11.1
PTS: 1
OBJ: 11.2; G2
3) ANS:
sublimation
DIF: 1
REF: Page Ref: 11.2
PTS: 1
DIF: 1
OBJ: 11.4; G2
4) ANS:
cholesteryl benzoate
REF: Page Ref: 11.4
PTS: 1
OBJ: 11.7; G2
DIF: 2
REF: Page Ref: 11.7
TRUE/FALSE
1) ANS:
OBJ:
2) ANS:
OBJ:
3) ANS:
OBJ:
4) ANS:
OBJ:
5) ANS:
OBJ:
F
PTS:
11.2; G2
T
PTS:
11.2; G2
T
PTS:
11.4; G2
T
PTS:
11.5, 11.6; G2
T
PTS:
11.7; G2
1
DIF: 2
REF: Page Ref: 11.2
1
DIF: 2
REF: Page Ref: 11.2
1
DIF: 1
REF: Page Ref: 11.4
1
DIF: 2
REF: Page Ref: 11.6
1
DIF: 2
REF: Page Ref: 11.7
2
Unit 11 Practice [Answer Strip]
C
_____
7)
B
_____
1)
ID: A
C 11)
_____
B 12)
_____
A
_____
8)
C
_____
2)
C 17)
_____
A 13)
_____
A 15)
_____
D
_____
3)
E 14)
_____
E 18)
_____
A
_____
4)
C 19)
_____
A
_____
9)
A 20)
_____
E
_____
5)
B 10)
_____
A
_____
6)
A 16)
_____
A 21)
_____
Unit 11 Practice [Answer Strip]
ID: A
T
_____
2)
A 22)
_____
T
_____
3)
T
_____
4)
A 23)
_____
T
_____
5)
B 24)
_____
E 26)
_____
D 25)
_____
F
_____
1)

Download Report